Microwave-Assisted Synthesis of Flower-like MnMoO4 Nanostructures and Their Photocatalytic Performance

This article describes an affordable method for the synthesis of MnMoO4 nanoflowers through the microwave synthesis approach. By manipulating the reaction parameters like solvent, pH, microwave power, and irradiation duration along this pathway, various nanostructures can be acquired. The synthesized nanoflowers were analyzed by using a powder X-ray diffractometer (XRD), field emission scanning electron microscopy (FE-SEM) with energy dispersive X-ray spectroscopy (EDS), Fourier transform infrared spectroscopy (FT-IR), and UV–vis diffuse reflectance spectroscopy (UV–DRS) to determine their crystalline nature, morphological and functional group, and optical properties, respectively. X-ray photoelectron spectroscopy (XPS) was performed for the examination of elemental composition and chemical states by qualitative and quantitative analysis. The results of the investigations demonstrated that the MnMoO4 nanostructures with good crystallinity and distinct shape were formed successfully. The synthesized MnMoO4 nanoflowers were tested for their efficiency as a photocatalyst in the degradation studies of methylene blue (MB) as model organic contaminants in an aqueous medium under visible light, which showed their photocatalytic activity with a degradation of 85%. Through the band position calculations using the electronegative value of MnMoO4, the photocatalytic mechanism of the nanostructures was proposed. The results indicated that the effective charge separation, and transfer mechanisms, in addition to the flower-like shape, were responsible for the photocatalytic performance. The stability of the recovered photocatalyst was examined through its recyclability in the degradation of MB. Leveraging MnMoO4’s photocatalytic properties, future studies may focus on scaling up these processes for practical and large-scale environmental remediation.


Introduction
Poisonous and dangerous substances affect the ecological integrity and ecosystems of the globe, necessitating comprehensive environmental organization and rehabilitation [1].The persistence, non-biodegradability, and bioaccumulation of numerous biochemical pollutants endanger social wellbeing and reduce financial wellbeing, creating significant problems for environmental groups.The rapid industrial expansion, fueled by unsustainable technical breakthroughs, can result in industrial wastewater, which is generated in significant quantities worldwide each year, increasing chemical risks [2].These substances have been strongly connected to significant consequences and long-term impacts, the majority of which are related to acute water poisoning.To address the quick identification and detection of these problematic substances, proper risk assessment methodologies are required [3].The contamination of water is caused by a variety of pollutants, including inorganic (salts, caustic metal ions, and metal oxides) and organic (pesticides, fertilizers, phenol, and dyes) pollutants, agricultural runoff, and so on [4][5][6].The methods for removing organic matter can be distinctly separated into three groups: (i) physical, (ii) chemical, and (iii) biological, which include precipitation [7], ion exchange [8], sonochemical degradation [9], adsorption [10], and various advanced oxidation process techniques such as Fenton [11], photo-Fenton [12], photocatalysis [13], etc.
The degradation of environmental contaminants using photocatalysis is an interesting approach.With its capacity to break down different pollutants and convert light energy into chemical energy, photocatalysis has captured the attention of researchers studying possible applications of today's technological advancements.This opens up promising avenues for the removal of potentially dangerous contaminants from the environment [14,15].Photocatalysis is the succession of the oxidation and reduction processes caused by electrons and holes stimulated by photons.The photocatalytic performance of the catalysts will eventually be linked with its shape, chemical and surface characteristics, and crystallinity.Hence, using the photocatalysis approach as a strategy for water purification necessitates the active use of UV and visible light, as well as the usage of highly complicated photocatalysts.The development of a photocatalysis system that counteracts the visible and UV light is critical for removing organic pollutants from the wastewater [16,17].
Molybdenum (Mo)-based nanomaterials have been largely studied in the field of photocatalytic pollutant degradation.They have been extensively used as environmental remediation materials because of their exceptional performance in photocatalysis.Molybdenum oxides have garnered significant attention in recent times for their potential applications in several domains, such as humidity sensors, magnetic fields, the microwave approach, optical fibers, scintillator materials, photoluminescence devices, catalysis, and electrochemical sensors, owing to their physiochemical characteristics [18][19][20][21].Adding certain precious metals to the oxides can enhance their optical, catalytic, and sensing properties.In recent decades, several metal molybdates with various shapes and characteristics have been documented [22].Molybdates are compounds containing molybdenum oxy anions in which molybdenum has the formal oxidation number of +6.Molybdates are a significant group of transition metal oxides.They possess an extremely large bivalent cation with an ionic radius >0.99 for scheelite structures, such those of Ba, Sr, Pb, or Ca.In this way, the binary metal oxide manganese molybdate (MnMoO 4 ) has received a lot of research interest recently because of its affordability, viability as oxidation states, improved electrical conductivity, and good thermal and chemical stability, allowing it to achieve superior electrochemical performance [23,24].
Additionally, a wide range of rich redox reactions are offered by the metal ions in binary metal oxides.Among the binary metal oxides, MnMoO 4 has attracted a lot of attention due to its low cost, environmental friendliness, excellent electrical conductivity, broad working voltage window, and remarkable stability.Furthermore, MnMoO 4 exhibits outstanding qualities including natural abundance, low toxicity, and a stable crystal structure.Its enormous theoretical specific capacitance and strong electrical conductivity make it environmentally beneficial.The binary metal naturally has a wide operating voltage window and a high retention capacity for energy storage devices [25].
In the present investigation, the microwave synthesis methodology was utilized for the production of MnMoO 4 .The morphology of synthesized MnMoO 4 was confirmed to be flower-like structures.The structural and optical properties of synthesized MnMoO 4 were confirmed and the phase validation was performed.The synthesized catalyst was utilized for the degradation of methylene blue (MB) through the photocatalytic degradation process as a representative organic toxin.

Materials and Methods
The basic starting materials used in the synthesis of MnMoO 4 such as manganese acetate Mn(CH 3 CO 2 ) 2 •(H 2 O), ammonium molybdate ((NH 4 ) 6 Mo 7 O 24 ), and methylene blue (MB) were analytical grade chemicals acquired from SRL, India.Two solvents were utilized in the synthesis process: ethanol and double-distilled water (DDW).

Synthesis of MnMoO 4 Flowers
The simple microwave approach was used for producing MnMoO 4 flowers.The typical methodology involved dissolving 2 mmol of Mn(CH 3 CO 2 ) 2 •(H 2 O) in 30 mL of polyethylene glycol and 0.27 mmol of ammonium molybdate in 30 mL of polyethylene glycol separately at 70 • C, with each solution named as solution A and solution B. Both the solutions were added to each other drop by drop.The pH of the reaction medium was brought to 11 through introducing ethylenediamine; the suspension was subjected to microwave radiation at 750 W for 7 min.The final sample was cleaned multiple times with DDW and ethanol before being oven-dried for 6 h at 90 • C. The resultant powder was ultimately calcined for 2 h at 500 • C to obtain the crystalline MnMoO 4 nanoflowers.

MnMoO 4 Nanoflower Investigated with Different Characterizations
The XRD method was used to determine the sample's crystallinity, and a Rich Siefert 3000 diffractometer was used to measure the sample's response to Cu-K α1 radiation (λ = 1.5406).X-ray photoelectron spectroscopy (XPS) performed by Omicron nanotechnology-ESCA-14, Germany, was employed to define the chemical structure of the manganese molybdate.The FT-IR spectroscopic analysis (using a Perkin-Elmer spectrophotometer) was used to examine the compound's functional group.For the sample analysis, the KBr pellet technique was employed.The Raman-11 Nano Photon Corporation Instrument, manufactured in Japan, was utilized for the Raman analysis.Using a Perkin-Elmer spectrophotometer, the material's optical properties were evaluated.By using field emission scanning electron microscopy (FE-SEM), HITACHI SU6600, FEI, Hitachi High-Technologies, Tokyo, Japan, the morphology of manganese molybdate was recorded.  .The synthesized material is highly crystalline in nature, as seen through the strong diffraction of MnMoO 4 .Furthermore, there were no further impurity peaks found [26].

Structural Analysis by XRD
synthesized material is highly crystalline in nature, as seen through the strong diffraction of MnMoO4.Furthermore, there were no further impurity peaks found [26].

XPS Investigation
The MnMoO4 nanostructures were subjected to XPS examination in order to verify the elements' oxidation states, binding energies, and chemical composition.The survey XPS spectrum of MnMoO4 is displayed in Figure 2a.It displays the occurrence of Mn, Mo, and O in the produced MnMoO4.This outcome aligns with the EDAX study.Additionally, the following section discusses the high-resolution XPS spectra of the produced MnMoO4 nanoflowers for Mn 2p, Mo 3d, and O 1s.The XPS spectrum of Mn 2p is shown in Figure 2b.Doublet peaks are seen at 641.5 and 653.7 eV, respectively, which correspond to Mn 2p3/2 and Mn 2p1/2.This indicates that the oxidation state of +2 of the Mn in the sample is present.The Mo 3d XPS spectrum is seen in Figure 2c, with two peaks at 228.4 and 231.5 eV, respectively, that belong to Mo 3d.The measured Mo 3d3/2 and Mo 3d5/2 doublets' separation was found to be 3.1 eV, corresponding to the Mo +6 oxidation state [27,28].The O 1s peak has a prominent component centered at 529.2 eV with a low binding energy; this is indicative of the oxide that forms O 2-with components of manganese and molybdenum (Mn-O-Mo), and 531.9 eV corresponds to the surface hydroxyl group, as shown in Figure 2d [29].The C1s peak is fi ed with two peaks at 285.6 and 289.3 eV which belong to C 1s and C-O, respectively [30].Further, by referring to the previous literature, quantification of the synthesized catalyst MnMoO4 is calculated.Mn, Mo, and O elements are displayed along with an error bar in atomic % from the high-resolution XPS spectra; the relevant values are provided in Table 1 [31].

XPS Investigation
The MnMoO 4 nanostructures were subjected to XPS examination in order to verify the elements' oxidation states, binding energies, and chemical composition.The survey XPS spectrum of MnMoO 4 is displayed in Figure 2a.It displays the occurrence of Mn, Mo, and O in the produced MnMoO 4 .This outcome aligns with the EDAX study.Additionally, the following section discusses the high-resolution XPS spectra of the produced MnMoO 4 nanoflowers for Mn 2p, Mo 3d, and O 1s.The XPS spectrum of Mn 2p is shown in Figure 2b.Doublet peaks are seen at 641.5 and 653.7 eV, respectively, which correspond to Mn 2p 3/2 and Mn 2p 1/2 .This indicates that the oxidation state of +2 of the Mn in the sample is present.The Mo 3d XPS spectrum is seen in Figure 2c, with two peaks at 228.4 and 231.5 eV, respectively, that belong to Mo 3d.The measured Mo 3d 3/2 and Mo 3d 5/2 doublets' separation was found to be 3.1 eV, corresponding to the Mo +6 oxidation state [27,28].The O 1s peak has a prominent component centered at 529.2 eV with a low binding energy; this is indicative of the oxide that forms O 2-with components of manganese and molybdenum (Mn-O-Mo), and 531.9 eV corresponds to the surface hydroxyl group, as shown in Figure 2d [29].The C1s peak is fitted with two peaks at 285.6 and 289.3 eV which belong to C 1s and C-O, respectively [30].Further, by referring to the previous literature, quantification of the synthesized catalyst MnMoO 4 is calculated.Mn, Mo, and O elements are displayed along with an error bar in atomic % from the high-resolution XPS spectra; the relevant values are provided in Table 1 [31].

Structural and Optical Properties
Figure 3a displays the synthesized MnMoO4 Raman spectrum.The measured band for the synthesized MnMoO4 correspond to the different modes.MnMoO4 was found have bands at 902, 782, 542, 402, 338, and 273 cm −1 .The Raman peaks at 902 and 782 cm are caused by symmetrical stretching of Mo-O-Mo and asymmetrical stretching of υ Mo=O [32].The Mo-O-Mo bond, which is due to mutual oxygen atoms of 2 and 3 octah dral MoO6, due to symmetric and asymmetric stretching, is confirmed by peaks at 542 an 402 cm −1 [33].The signal that was seen at 273 cm −1 is consistent with the double bon O=Mo=O in MnMoO4 nanostructures due to wagging. Figure 3b shows the FT-IR spect of the synthesized MnMoO4.The surface hydroxyl O-H bond vibration is shown by a wid band seen at 3436 cm −1 .The H-O-H distortion mode of the surface hydroxyl assembly represented by the band at 1637 cm −1 [34].Peaks of MnMoO4 are seen at around 864 an 910 cm −1 , which corresponded to the stretching and bending vibration of Mo=O and Mo O-Mo, respectively.The optical property of produced MnMoO4 was examined using UV vis diffuse reflectance spectroscopy (DRS) and the obtained result is presented in Figu 2c.The robust absorption peak at 303 nm is due to the switch among bands of O 2p an Mn 3d levels in the MnMoO4 [35].The bandgap (Eg) of the manufactured MnMoO4 w calculated through Tauc's plot (Equation (1)).
(hυα) 1/n = A(hυ − Eg) ( The synthesized MnMoO4 presented a direct bandgap of 2.59 eV, which is shown Figure 3c,d [36].Additionally, the conduction band (CB) and valence band (VB) position were identified by using Equations ( 2) and (3): EVB = X − E e + 0.5Eg (   [32].The Mo-O-Mo bond, which is due to mutual oxygen atoms of 2 and 3 octahedral MoO 6 , due to symmetric and asymmetric stretching, is confirmed by peaks at 542 and 402 cm −1 [33].The signal that was seen at 273 cm −1 is consistent with the double bond O=Mo=O in MnMoO 4 nanostructures due to wagging. Figure 3b shows the FT-IR spectra of the synthesized MnMoO 4 .The surface hydroxyl O-H bond vibration is shown by a wide band seen at 3436 cm −1 .The H-O-H distortion mode of the surface hydroxyl assembly is represented by the band at 1637 cm −1 [34].Peaks of MnMoO 4 are seen at around 864 and 910 cm −1 , which corresponded to the stretching and bending vibration of Mo=O and Mo-O-Mo, respectively.The optical property of produced MnMoO 4 was examined using UV-vis diffuse reflectance spectroscopy (DRS) and the obtained result is presented in Figure 2c.The robust absorption peak at 303 nm is due to the switch among bands of O 2p and Mn 3d levels in the MnMoO 4 [35].The bandgap (E g ) of the manufactured MnMoO 4 was calculated through Tauc's plot (Equation ( 1)).

Structural and Optical Properties
(hυα The synthesized MnMoO 4 presented a direct bandgap of 2.59 eV, which is shown in Figure 3c,d [36].Additionally, the conduction band (CB) and valence band (VB) positions were identified by using Equations ( 2) and (3): The conduction band (CB) edge potential is denoted by E CB , the bandgap energy is represented by E g , the valence band (VB) edge potential is represented by E VB , and the electronegativity of MnMoO 4 is represented by X (5.94 eV).The E CB value for the MnMoO 4 flowers is determined to be −0.305eV using these calculations.Furthermore, the E VB value is estimated as 1.26 eV.The oxygen vacancies' role in the valence band edge increasing and the conduction band edge reducing is verified by these computations.To enable effective photocatalytic activity, the oxygen vacancies ideally stimulate the creation of sub-bands (below but near to CB) that both limit electron-hole recombination and function as amplifiers for the shift of electrons.

ECB=EVB − Eg
(3) The conduction band (CB) edge potential is denoted by ECB, the bandgap energy is represented by Eg, the valence band (VB) edge potential is represented by EVB, and the electronegativity of MnMoO4 is represented by X (5.94 eV).The ECB value for the MnMoO4 flowers is determined to be −0.305eV using these calculations.Furthermore, the EVB value is estimated as 1.26 eV.The oxygen vacancies' role in the valence band edge increasing and the conduction band edge reducing is verified by these computations.To enable effective photocatalytic activity, the oxygen vacancies ideally stimulate the creation of subbands (below but near to CB) that both limit electron-hole recombination and function as amplifiers for the shift of electrons.

Morphological Analysis
The FE-SEM images of MnMoO4 revealed the formation of flower-like structures, as shown in Figure 4a-d.These nanoflowers exhibited a high degree of MnMoO4 nanopetal arrangement to form a uniform flower-like morphology with size of 1 µm.The MnMoO4 nanoflowers are assembled from discrete nanopetals with a thickness of a nanometer [37].This hierarchical flower has more dense petals which may favor the photocatalytic activity due to the involvement of a greater number of nanopetals at a time.The EDS analysis (Figure 4d) confirmed the elemental composition of the MnMoO4 flowers.The spectrum displayed peaks corresponding to manganese (Mn), molybdenum (Mo), and oxygen (O), respectively.

Morphological Analysis
The FE-SEM images of MnMoO 4 revealed the formation of flower-like structures, as shown in Figure 4a-d.These nanoflowers exhibited a high degree of MnMoO 4 nanopetal arrangement to form a uniform flower-like morphology with size of 1 µm.The MnMoO 4 nanoflowers are assembled from discrete nanopetals with a thickness of a nanometer [37].This hierarchical flower has more dense petals which may favor the photocatalytic activity due to the involvement of a greater number of nanopetals at a time.The EDS analysis (Figure 4d) confirmed the elemental composition of the MnMoO 4 flowers.The spectrum displayed peaks corresponding to manganese (Mn), molybdenum (Mo), and oxygen (O), respectively.

Photodegradation of MB in the Presence of MnMoO4
Figure 5A portrays the photocatalytic action of the manufactured MnMoO4 flowers studied regarding the breakdown of methylene blue (MB) dye in the presence of visible light irradiation.Two types of control experiments were conducted by taking a blank dye (MB) solution of 1 × 10 −5 and a dye with MnMoO4 in dark conditions to compare the photocatalytic action of the material in the existence of light.The typical procedure of combining dye with a catalyst in the presence of light involves the addition of 100 mL of a 1 × 10 −5 M MB dye solution to a 250 mL beaker along with 50 mg of the catalyst (MnMoO4).The mixture of pollutant and catalyst was obtained in the dark, preventing contact with light, to achieve the adsorption-desorption balance of the photocatalyst and dye [38,39].Among the above two reaction mixtures, the pure dye solution and the dye with the catalyst were maintained in the dark, the dye was set with light, and the material with dye was exposed to the visible light after half an hour while being constantly stirred with magnetic stirrer.At regular intervals of every 10 min, all of the three sets of reaction mixture were collected by using a syringe filter to avoid sample contamination during UV-vis analysis.Figure 5B shows the C/C0 vs time plot of methylene blue in the dark, methylene blue in light, and methylene blue in the dark and light exposure condition in the presence of the photocatalyst.The color of the MB solution changes from dark blue to leucomethylene blue (colorless) as the MB decrease happens, which demonstrates the photodegradation plot of the pollutant molecules proposed by observing the decrease in the pollutant content under solar light.Firstly, the degradation of the MB solution was estimated in the absence of light to observe the chemical progression in the absence of light.Upon illumination, the pollutant concentration was gradually removed through photoreaction; the concentration in the dye deprived of any catalyst was noted to be 2.9% at 50 min, and the dye with the catalyst in the dark condition displayed the adsorption of the pollutant on the outer layer of catalyst, with the concentration being 13% at 50 min [40].As the photocatalyst reaction proceeds with the MnMoO4 flowers as the photocatalyst, it was seen that the absorption maximum of the dye peaks at 665 nm, reducing gradually at 50 min, with 85% of the dye observed, as shown in Figure 6a.The photocatalytic property of the present

Photodegradation of MB in the Presence of MnMoO 4
Figure 5A portrays the photocatalytic action of the manufactured MnMoO 4 flowers studied regarding the breakdown of methylene blue (MB) dye in the presence of visible light irradiation.Two types of control experiments were conducted by taking a blank dye (MB) solution of 1 × 10 −5 and a dye with MnMoO 4 in dark conditions to compare the photocatalytic action of the material in the existence of light.The typical procedure of combining dye with a catalyst in the presence of light involves the addition of 100 mL of a 1 × 10 −5 M MB dye solution to a 250 mL beaker along with 50 mg of the catalyst (MnMoO 4 ).The mixture of pollutant and catalyst was obtained in the dark, preventing contact with light, to achieve the adsorption-desorption balance of the photocatalyst and dye [38,39].Among the above two reaction mixtures, the pure dye solution and the dye with the catalyst were maintained in the dark, the dye was set with light, and the material with dye was exposed to the visible light after half an hour while being constantly stirred with magnetic stirrer.At regular intervals of every 10 min, all of the three sets of reaction mixture were collected by using a syringe filter to avoid sample contamination during UV-vis analysis.Figure 5B shows the C/C 0 vs time plot of methylene blue in the dark, methylene blue in light, and methylene blue in the dark and light exposure condition in the presence of the photocatalyst.The color of the MB solution changes from dark blue to leucomethylene blue (colorless) as the MB decrease happens, which demonstrates the photodegradation plot of the pollutant molecules proposed by observing the decrease in the pollutant content under solar light.Firstly, the degradation of the MB solution was estimated in the absence of light to observe the chemical progression in the absence of light.Upon illumination, the pollutant concentration was gradually removed through photoreaction; the concentration in the dye deprived of any catalyst was noted to be 2.9% at 50 min, and the dye with the catalyst in the dark condition displayed the adsorption of the pollutant on the outer layer of catalyst, with the concentration being 13% at 50 min [40].As the photocatalyst reaction proceeds with the MnMoO 4 flowers as the photocatalyst, it was seen that the absorption maximum of the dye peaks at 665 nm, reducing gradually at 50 min, with 85% of the dye observed, as shown in Figure 6a.The photocatalytic property of the present catalyst is matched with that previously stated in the literature and currently proposed in Table 2.
Materials 2024, 17, x FOR PEER REVIEW 8 of 12 catalyst is matched with that previously stated in the literature and currently proposed in Table 2.    catalyst is matched with that previously stated in the literature and currently proposed in Table 2.

Cycling Test to Remove Pollutants Using Photocatalysis
The photodegradation and stability of MnMoO 4 flowers toward MB dye was examined under identical reaction conditions.The MnMoO 4 photocatalyst was separated after the degrading process and given a thorough deionized water and ethanol wash.Before using the recovered catalyst in a second run, it was desiccated at 100 • C in a hot-air oven.The MB dye deterioration during the four runs is displayed in Figure 6b.In the consecutive four cycles with MnMoO 4 flowers, the MB dye degradation percentages were 85.00, 84.50, 83.29, and 83.00, respectively, with a 50 min reaction runtime.The MnMoO 4 flowers deterioration efficiency was not altered significantly, even after the consecutive four tests.Stability and reusability are essential components for a photocatalyst to be used in practical applications.The structural consistency of the MnMoO 4 flowers was tested later through X-ray diffraction analysis and morphological studies after four cycles; the obtained results are presented in Figure 7a,b.These results demonstrate that except from a decline in peak strength, morphology, and repeatable action, there are no observable structural changes during the photocatalytic processes.Consequently, it is possible to utilize wastewater management schemes for a long time.

Cycling Test to Remove Pollutants Using Photocatalysis
The photodegradation and stability of MnMoO4 flowers toward MB dye was examined under identical reaction conditions.The MnMoO4 photocatalyst was separated after the degrading process and given a thorough deionized water and ethanol wash.Before using the recovered catalyst in a second run, it was desiccated at 100 °C in a hot-air oven.The MB dye deterioration during the four runs is displayed in Figure 6b.In the consecutive four cycles with MnMoO4 flowers, the MB dye degradation percentages were 85.00, 84.50, 83.29, and 83.00, respectively, with a 50 min reaction runtime.The MnMoO4 flowers deterioration efficiency was not altered significantly, even after the consecutive four tests.Stability and reusability are essential components for a photocatalyst to be used in practical applications.The structural consistency of the MnMoO4 flowers was tested later through X-ray diffraction analysis and morphological studies after four cycles; the obtained results are presented in Figure 7a,b.These results demonstrate that except from a decline in peak strength, morphology, and repeatable action, there are no observable structural changes during the photocatalytic processes.Consequently, it is possible to utilize wastewater management schemes for a long time.

Conclusions
The microwave-assisted synthesis process was used to create the flower-like structured MnMoO4.XRD examination was utilized to confirm the monoclinic phase structure and the crystalline environment of the synthesized MnMoO4 flowers.Further, the chemical bonding of the molecule and the functional group identification of the MnMoO4 flowers were characterized via XPS, FTIR, and Raman analyses.The direct bandgap of 2.3 eV of the MnMoO4 was determined from the UV vis-DRS analysis and the flower-like structured morphology of the MnMoO4 was observed from the FE-SEM analysis.Finally, the produced material was studied for cycle stability and photocatalytic degradation effectiveness toward the organic pollutant MB dye with an irradiation time of 50 min with 85% of the degradation efficiency.Further, the stability of the synthesized photocatalyst was assessed by executing four consecutive runs of the photocatalyst experiments.Also, to investigate its durability, the FE-SEM and XRD analyses were employed with the postexperimental photocatalyst samples.The post-experimental samples exhibited almost the same morphology and crystal structure, with only a small decline in their peak intensities.

Conclusions
The microwave-assisted synthesis process was used to create the flower-like structured MnMoO 4 .XRD examination was utilized to confirm the monoclinic phase structure and the crystalline environment of the synthesized MnMoO 4 flowers.Further, the chemical bonding of the molecule and the functional group identification of the MnMoO 4 flowers were characterized via XPS, FTIR, and Raman analyses.The direct bandgap of 2.3 eV of the MnMoO 4 was determined from the UV vis-DRS analysis and the flower-like structured morphology of the MnMoO 4 was observed from the FE-SEM analysis.Finally, the produced material was studied for cycle stability and photocatalytic degradation effectiveness toward the organic pollutant MB dye with an irradiation time of 50 min with 85% of the degradation efficiency.Further, the stability of the synthesized photocatalyst was assessed by executing four consecutive runs of the photocatalyst experiments.Also, to investigate its durability, the FE-SEM and XRD analyses were employed with the post-experimental photocatalyst samples.The post-experimental samples exhibited almost the same morphology and crystal structure, with only a small decline in their peak intensities.Thus, the synthesized MnMoO 4 flower-like structured photocatalysts could be highly suitable as applications in wastewater treatment for a longer duration.

Figure 2 .
Figure 2. The XPS (a) survey spectrum of MnMoO4; (b-e) core-level spectrum of Mn, Mo, O, and C, respectively.

Figure 3a displays the synthesized MnMoO 4
Figure 3a displays the synthesized MnMoO 4 Raman spectrum.The measured bands for the synthesized MnMoO 4 correspond to the different modes.MnMoO 4 was found to have bands at 902, 782, 542, 402, 338, and 273 cm −1 .The Raman peaks at 902 and 782 cm −1 are caused by symmetrical stretching of Mo-O-Mo and asymmetrical stretching of υ as Mo=O[32].The Mo-O-Mo bond, which is due to mutual oxygen atoms of 2 and 3 octahedral MoO 6 , due to symmetric and asymmetric stretching, is confirmed by peaks at 542 and 402 cm −1[33].The signal that was seen at 273 cm −1 is consistent with the double bond O=Mo=O in MnMoO 4 nanostructures due to wagging.Figure3bshows the FT-IR spectra of the synthesized MnMoO 4 .The surface hydroxyl O-H bond vibration is shown by a wide band seen at 3436 cm −1 .The H-O-H distortion mode of the surface hydroxyl assembly is represented by the band at 1637 cm −1[34].Peaks of MnMoO 4 are seen at around 864 and 910 cm −1 , which corresponded to the stretching and bending vibration of Mo=O and Mo-O-Mo, respectively.The optical property of produced MnMoO 4 was examined using UV-vis diffuse reflectance spectroscopy (DRS) and the obtained result is presented in Figure2c.The robust absorption peak at 303 nm is due to the switch among bands of O 2p and Mn 3d levels in the MnMoO 4[35].The bandgap (E g ) of the manufactured MnMoO 4 was calculated through Tauc's plot (Equation (1)).

Figure 3 .
Figure 3. (a-d) The Raman, FT-IR, and DRS-UV spectra corresponding to the bandgap of the prepared MnMoO4 flowers.

Figure 3 .
Figure 3. (a-d) The Raman, FT-IR, and DRS-UV spectra corresponding to the bandgap of the prepared MnMoO 4 flowers.

Figure 4 .
Figure 4. (a-c) The FE-SEM images of MnMoO4 and (d) the corresponding EDS.

Figure 4 .
Figure 4. (a-c) The FE-SEM images of MnMoO 4 and (d) the corresponding EDS.

Figure 5 .
Figure 5. (A) The absorption spectra of methylene blue degradation with MnMoO4 flowers from 0 to 50 min (represented by (a) to (f)) during photocatalysis, and (B) C/C0 vs. time plot of methylene blue.

Figure 6 .
Figure 6.(a) The degradation efficacy % with respect to time; (b) the cycling test of the photocatalytic degradation of pollutants on MnMoO4 flowers.

Figure 5 .
Figure 5. (A) The absorption spectra of methylene blue degradation with MnMoO 4 flowers from 0 to 50 min (represented by (a) to (f)) during photocatalysis, and (B) C/C 0 vs. time plot of methylene blue.

Figure 5 .Figure 6 .
Figure 5. (A) The absorption spectra of methylene blue degradation with MnMoO4 flowers from 0 to 50 min (represented by (a) to (f)) during photocatalysis, and (B) C/C0 vs. time plot of methylene

Figure 6 .
Figure 6.(a) The degradation efficacy % with respect to time; (b) the cycling test of the photocatalytic degradation of pollutants on MnMoO 4 flowers.

Figure 7 .
Figure 7. (a) The XRD pa erns and (b) the FE-SEM analysis of MnMoO4 flowers synthesized and after catalytic reaction.

Figure 7 .
Figure 7. (a) The XRD patterns and (b) the FE-SEM analysis of MnMoO 4 flowers synthesized and after catalytic reaction.

Table 1 .
Atomic % of the elements present in MnMoO 4 .

Table 1 .
Atomic % of the elements present in MnMoO4.

Table 2 .
Comparison with other photocatalysts for the degradation of MB.

Table 2 .
Comparison with other photocatalysts for the degradation of MB.

Table 2 .
Comparison with other photocatalysts for the degradation of MB.